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- O-H H CH,OH (b) CH2 CH, NH, H--0=C (b) 0-H-- (a) CH, CH, CH, CH H-C CH, (CH.)4–NH, CH, CH, |(d) (a) CH, (d) (c) CH, CH, HC CH CH, CH,COOH (b) [The image above is from a different textbook. Ask me later if you would like to know the reference.] The image above depicts protein tertiary structure. What type of tertiary structure is represented by the letter (d) in the image? O hydrogen bonding 3 of these 4 responses are correct. O disulfide linkage O hydrophobic interaction salt bridge(A) + H20 oH (B)52 (a)
- Calculate the equilibrium constant for the acid–base reaction between the reactants in each of the following pairs: (a) HCl + H2O (b) CH3COOH + H2O (c) CH3NH2 + H2O (d) CH3N+H3 + H2O(a) (b) (c) t2-11 2.19] A solution has an H+ concentration of 10-5 M. (a) What is the pH of this solution? (b) What is the pOH (Assume that the temperature of the solution is 25°C.) Answer: (a) 5 (b) 9 BM
- HO 1) 2) OHWhen ammonium sulfate dissolves, both the anion and cation have acid-base reaction: (NH4)2SO4(s) 2NH4* + SO42- NH4* + NH3(aq) + H* SO2- + H2O → HSO4 + OH Ksp = 276 Ka = 5.70 x10-10 Кь 3 9.80 х 10-13 (a) (b) (c) Write a charge balance for this system. Write a mass balance for this system. Find the concentration of NH3(aq) if the pH is fixed at 9.25.What is the basis for referring to the hydrogen ion as a proton? (a) The Arrhenius definition of an acid. (b) The Brønsted-Lowry definition of an acid x (c) The Lewis definition of an acid. (d) H* exists as a bare proton. (e) None of these.
- (a) (1) CI AICI (2) HNO₂, H₂SO (3) O (4) Me,S (5) NaBH; H₂O+ एल Draw Your SolutionWhich of the following is a strong acid in aqueous solution? (a) Mg(OH)2 (b) NH3 (c) H2SO4 (d) CH3COOH (e) AgClAmmonia, NH3, is amphoteric. (a) Give the formula for the conjugate acid of NH3. (b) Give the formula for the conjugate base of NH3.